![]() So we have hydrogen is at 1.008, and then we have carbon, and carbon is at 12.01. We can see hydrogen has anĪverage atomic mass of 1.008. So I'll get out our handy periodic table. Of a molecule or an atom, let's just get the average atomic mass for carbon, hydrogen, and I'm going to be thinking about molar moles and molar masses and the mass of a mole ![]() Hydrogen did we start with? And if we look at those ratios, then we can come up with Out how many moles of carbon dioxide we have, how many moles of water we have, and from that, we canįigure out how many moles of carbon did we start with and how many moles of And so what we need toĭo is say, all right, from that, we can figure They tell us how many grams of the carbon dioxide we have and how many grams of the water we have, they tells us that right over there. I could try to, even with the x's and y's, but that's not the point of this video. ![]() And what I just drew here, this is a chemical reaction ![]() Presence of molecular oxygen and it's going to combust and after it's combusted, I'm going to end up with someĬarbon dioxide and some water. It only contains carbon and hydrogen, so it's going to have To make sure we understand what's going on. ![]() What is the empiricalįormula of the compound? So pause this video and see if you can work through that. That a sample of a compound containing only carbon and hydrogen atoms is completely combusted, producing 5.65 grams of carbon dioxide and 3.47 grams of H2O or water. ![]()
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